A sculptor has asked you to help electroplate gold onto a brass statue. You know that the charge carriers in the ionic solution are monovalent (charge e) gold ions, and you've calculated that you must deposit 0.60 g of gold to reach the necessary thickness.

How much current do you need, in mA, to plate the statue in 3.5 hr?

The current needed, in mA, to plate the statue in 3.5 hr is 20 mA

Explanation:

Moles of electron = 1 mole

According to mole concept:

1 mole of an atom contains number of particles.

We know that:

Charge on 1 electron =

Charge on 1 mole of electrons =

197 g of gold is deposited by = 96500 C of electricity

Thus 0.60 g of gold is deposited by = of electricity

To calculate the current required, we use the equation:

where,

I = current passed = ?

q = total charge =

t = time required = 3.5 hrs =

Putting values in above equation, we get:

Hence, the current needed, in mA, to plate the statue in 3.5 hr is 20 mA

a chemical reaction happens

explanation:

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